Carbon monofluoride

Fig. 1. Stmcture of poly(carbon monofluoride). , carbon o, fluorine. The interstitial space is 0.66 nm.

Graphite fluoride continues to be of interest as a high temperature lubricant (6). Careful temperature control at 627 3° C results in the synthesis of poly(carbon monofluoride) [25136-85-0] (6). The compound remains stable in air to ca 600°C and is a superior lubricant under extreme conditions of high temperatures, heavy loads, and oxidising conditions (see Lubrication and lubricants). It can be used as an anode for high energy batteries (qv). 

Leclanche or dry cell Alkaline Cell Silver-Zinc Reuben Cell Zinc-Air Fuel Cell Lithium Iodine Lithium-Sulfur Dioxide Lithium-Thionyl Chloride Lithium-Manganese Dioxide Lithium-Carbon Monofluoride... 

Table S, Specifications of coin-type lithium-carbon monofluoride batteries...

Catalogue of lithium-carbon monofluoride batteries, Matsushita Battery Industrial Co., Ltd., 1996. 

As a review on poly(carbon monofluoride) has recently appeared (K1), our treatment here will be cursory,... 

Made by direct combination of graphite and fluorine in the temperature range 420-630°C, carbon monofluoride is a white, nonconducting powder, chemically more similar to Teflon than to graphite. 

As with graphite oxide, there are currently two views as to the structure of carbon monofluoride. Although detailed X-ray diffraction work suggested a chair arrangement of the sp -hybridized, carbon sheets (Ml), second-moment calculations of the adsorption mode of the fluorine nuclear magnetic resonance suggested that a boat arrangement is more plausible iE2). The structures are illustrated in Fig. 3. 

Carbon monofluoride has found use as a lubricant. Studies by Fusaro and Sliney FI, F2) and Gisser (G2) showed that carbon monofluoride is superior to molybdenum disulfide under many conditions. Grafting of monomers can further improve lubricity (B4). Electrochemical applications are discussed later. 

Dining interaction at ambient temperature in a bomb to produce poly (carbon monofluoride), admission of fluorine beyond a pressure of 13.6 bar must be extremely slow and carefully controlled to avoid a violently exothermic explosion [1], Previously it had been shown that explosive interaction of carbon and fluorine was due to the formation and decomposition of the graphite intercalation compound, poly (carbon monofluoride) [2], Presence of mercury compounds prevents explosion during interaction of charcoal and fluorine [3], Reaction of surplus fluorine with graphite or carbon pellets was formerly used as a disposal method, but is no longer recommended. Violent reactions observed when an exhausted trap was opened usually involved external impact on the metal trap, prodding the trap contents to empty the trap, or possibly ingress of moist air... 

We are going to discuss the syntheses of fluoropolymers, poly(carbon monofluoride), perfluoropolyethers, perfluorinated nitrogen-containing ladder polymers, and surface fluorination of polymers by direct fluorination. 

Poly(carbon monofluoride), (CF ) (Figure 14.2) has been known since 1934 when Ruff and co-workers16 prepared a gray compound of composition CF0.92. In 1947 W. and G. Rodorff7,18 reported a series of compositions of CF0.68 to CF0.99, varying in color from black in the case of CF0 68 through gray to white in the case of CF0.99 ... 

Studies at the Lewis Research Center of the National Aeronautic and Space Administration22 and at the Frankford Arsenal of the U.S. Army23 have shown that poly(carbon monofluoride) is a superior solid lubricant under heavy loads, in high temperatures, in oxidizing atmospheres, and under other extreme conditions. Researchers at the U.S. Army Electronics Command at Fort Monmouth, N.J.24 25 and industrial scientists in Japan have recently demonstrated a high potential for the use of poly(carbon monofluoride) as a cathode material in high-energy batteries. 

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